Fe_{2}O_{3} + 6HCl → 2FeCl_{3} + 3H_{2}O

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### Word Equation

Hematite + Hydrogen Chloride = Ferric Chloride + Water

One mole of

and six moles of

react to lớn form two moles of

and three moles of

Place in the bottom of a test tube at the base oxide Fe2O3 1-2 ml of acid, then flick → The solid Đen Ferric oxide (Fe2O3) melting, creating golden brown solution

Fe2O3 generated acid reacts with iron salts (III) golden brown

### Reactants

### Hematite - Fe

_{2}O_{3}Iron(3+);Oxygen(2-) Haematitis Of Pliny Raphisiderite Oligiste Blood Stone

### Hydrogen Chloride - HCl

Hcl

### Products

### Ferric Chloride - FeCl

_{3}Fecl3 [Fecl3] Ferric;Trichloride Iron(3+);Trichloride

### Water - H

_{2}OHydroxic Acid H₂O [Oh2] Aqua Pure Water Hydrogen Oxide Oxidane Dihydrogen Oxide

### Thermodynamics

Thermodynamics of the reaction can be calculated using a lookup table.

#### Is the Reaction Exothermic or Endothermic?

Fe_{2}O_{3} (s hematite) | 1 mol | -824.248 kJ/mol | 824.248 kJ |
---|---|---|---|

HCl (g) | 6 mol | -92.29904 kJ/mol | 553.79424 kJ |

FeCl_{3} (s) | 2 mol | -399.48832 kJ/mol | -798.97664 kJ |

H_{2}O (g) | 3 mol | -241.818464 kJ/mol | -725.455392 kJ |

ΣΔH°_{f}(reactants) | -1378.04224 kJ | ||

ΣΔH°_{f}(products) | -1524.432032 kJ | ||

ΔH°_{rxn} | -146.389792 kJ |

ΣΔH°_{f}(reactants) > ΣΔH°_{f}(products), sánh Fe2O3 + HCl = FeCl3 + H2O is **exothermic** (releases heat).

#### Is the Reaction Exoentropic or Endoentropic?

ΔS = S_{products} - S_{reactants}. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.

Fe_{2}O_{3} (s hematite) | 1 mol | 87.40376 J/(mol K) | -87.40376 J/K |
---|---|---|---|

HCl (g) | 6 mol | 186.77376 J/(mol K) | -1120.64256 J/K |

FeCl_{3} (s) | 2 mol | 142.256 J/(mol K) | 284.512 J/K |

H_{2}O (g) | 3 mol | 188.715136 J/(mol K) | 566.145408 J/K |

ΣΔS°(reactants) | 1208.04632 J/K | ||

ΣΔS°(products) | 850.657408 J/K | ||

ΔS°_{rxn} | -357.388912 J/K |

ΣΔS°(reactants) > ΣΔS°(products), sánh Fe2O3 + HCl = FeCl3 + H2O is **exoentropic** (decrease in entropy).

#### Is the Reaction Exergonic or Endergonic?

ΔG = G_{products} - G_{reactants}. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.

Fe_{2}O_{3} (s hematite) | 1 mol | -742.2416 kJ/mol | 742.2416 kJ |
---|---|---|---|

HCl (g) | 6 mol | -95.31152 kJ/mol | 571.86912 kJ |

FeCl_{3} (s) | 2 mol | -334.05056 kJ/mol | -668.10112 kJ |

H_{2}O (g) | 3 mol | -228.588656 kJ/mol | -685.765968 kJ |

ΣΔG°(reactants) | -1314.11072 kJ | ||

ΣΔG°(products) | -1353.867088 kJ | ||

ΔG°_{rxn} | -39.756368 kJ |

ΣΔG°(reactants) > ΣΔG°(products), sánh Fe2O3 + HCl = FeCl3 + H2O is **exergonic** (releases energy).

### Reaction Expressions

K_{c} or Q = ( [FeCl_{3}]^{2} [H_{2}O]^{3} ) / ( [Fe_{2}O_{3}] [HCl]^{6} )

(assuming all reactants and products are aqueous. substitutue 1 for any solids/liquids, and Psubstance for gases.)

rate = -(Δ[Fe_{2}O_{3}] / Δt) = -1/6 * (Δ[HCl] / Δt) = 50% * (Δ[FeCl_{3}] / Δt) = 1/3 * (Δ[H_{2}O] / Δt)

(assuming constant volume in a closed system and no accumulation of intermediates or side products)

## Instructions

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To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. The balanced equation will appear above.

- Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F.
- Ionic charges are not yet supported and will be ignored.
- Replace immutable groups in compounds to lớn avoid ambiguity. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will.
- Compound states [like (s) (aq) or (g)] are not required.
- You can use parenthesis () or brackets [].

## How To Balance Equations

Read our article on how to lớn balance chemical equations or ask for help in our chat.

You can also ask for help in our chat or forums.

## Practice Balancing Fe2O3 + HCl = FeCl3 + H2O

## Balance Fe2O3 + HCl = FeCl3 + H2O Using the Algebraic Method

To balance the equation Fe2O3 + HCl = FeCl3 + H2O using the algebraic method step-by-step, you must have experience solving systems of linear equations. The most common methods are substitution/elimination and linear algebra, but any similar method will work.

### Step 1: Label Each Compound With a Variable

Label each compound (reactant or product) in the equation with a variable to lớn represent the unknown coefficients.

a Fe_{2}O_{3} + b HCl = c FeCl_{3} + d H_{2}O

### Step 2: Create a System of Equations

Create an equation for each element (Fe, O, H, Cl) where each term represents the number of atoms of the element in each reactant or product.

**Fe**: 2a + 0b = 1c + 0d
**O**: 3a + 0b = 0c + 1d
**H**: 0a + 1b = 0c + 2d
**Cl**: 0a + 1b = 3c + 0d

### Step 3: Solve For All Variables

Use substitution, Gaussian elimination, or a calculator to lớn solve for each variable.

- 2a - 1c = 0
- 3a - 1d = 0
- 1b - 2d = 0
- 1b - 3c = 0

Use your graphing calculator's rref() function (or an online rref calculator) to lớn convert the following matrix into reduced row-echelon-form:

[ 2 0 -1 0 0] [ 3 0 0 -1 0] [ 0 1 0 -2 0] [ 0 1 -3 0 0]

The resulting matrix can be used to lớn determine the coefficients. In the case of a single solution, the last column of the matrix will contain the coefficients.

Simplify the result to lớn get the lowest, whole integer values.

- a = 1 (Fe2O3)
- b = 6 (HCl)
- c = 2 (FeCl3)
- d = 3 (H2O)

### Step 4: Substitute Coefficients and Verify Result

Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.

Fe_{2}O_{3} + 6 HCl = 2 FeCl_{3} + 3 H_{2}O

Fe | 2 | 2 | ✔️ |
---|---|---|---|

O | 3 | 3 | ✔️ |

H | 6 | 6 | ✔️ |

Cl | 6 | 6 | ✔️ |

Since there is an equal number of each element in the reactants and products of Fe2O3 + 6HCl = 2FeCl3 + 3H2O, the equation is balanced.

## Balance Fe2O3 + HCl = FeCl3 + H2O Using Inspection

The law of conservation of mass states that matter cannot be created or destroyed, which means there must be the same number atoms at the kết thúc of a chemical reaction as at the beginning. To be balanced, every element in Fe2O3 + HCl = FeCl3 + H2O must have the same number of atoms on each side of the equation. When using the inspection method (also known as the trial-and-error method), this principle is used to lớn balance one element at a time until both sides are equal and the chemical equation is balanced.

### Step 1: Count the number of each element on the left and right hand sides

Reactants (Left Hand Side) | Products (Right Hand Side) | ||||||
---|---|---|---|---|---|---|---|

Reactants | Products | ||||||

Fe_{2}O_{3} | HCl | Total | FeCl_{3} | H_{2}O | Total | ||

Fe | 2 | 2 | 1 | 1 | ❌ | ||

O | 3 | 3 | 1 | 1 | ❌ | ||

H | 1 | 1 | 2 | 2 | ❌ | ||

Cl | 1 | 1 | 3 | 3 | ❌ |

### Step 2: Multiply coefficients for compounds to lớn balance out each element

For each element that is not equal, try to lớn balance it by adding more of it to lớn the side with less. Sometimes there may be multiple compounds with that element on one side, sánh you'll need to lớn use your best judgement and be prepared to lớn go back and try the other options.

**Fe**is not balanced. Add**1**molecule of**FeCl**to lớn the product (right-hand) side to lớn balance Iron:_{3}

Fe_{2}O_{3}+ HCl = 2FeCl_{3}+ H_{2}OReactants Products Fe 2 2 ✔️ O 3 1 ❌ H 1 2 ❌ Cl 1 6 ❌ **O**is not balanced. Add**2**molecules of**H**to lớn the product (right-hand) side to lớn balance Oxygen:_{2}O

Fe_{2}O_{3}+ HCl = 2FeCl_{3}+ 3H_{2}OReactants Products Fe 2 2 ✔️ O 3 3 ✔️ H 1 6 ❌ Cl 1 6 ❌ **H**is not balanced. Add**5**molecules of**HCl**to lớn the reactant (left-hand) side to lớn balance Hydrogen:

Fe_{2}O_{3}+ 6HCl = 2FeCl_{3}+ 3H_{2}OReactants Products Fe 2 2 ✔️ O 3 3 ✔️ H 6 6 ✔️ Cl 6 6 ✔️

### Step 3: Verify that the equation is balanced

Since there are an equal number of atoms of each element on both sides, the equation is balanced.

Fe_{2}O_{3} + 6HCl = 2FeCl_{3} + 3H_{2}O

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